The final molarity of a solution made by mixing $50 m L$ of $0.5 M H C l$ , $150 m L$ of $0.25 M$ $H C l$ and water to make the volume $250 m L$ is:

0.5 M

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1 M

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0.75 M

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0.25 M

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Solution

The correct option is D $0.25 M$
For a mixture of solution,
$M_{f} \times V_{f} = M_{1} V_{1} + M_{2} V_{2} + M_{3} V_{3} + . . .$
Given: $V_{1} = 50 m L, M_{1} = 0.5 M, V_{2} = 150 m L, M_{2} = 0.25 M, V_{f} = 250 m L$
$M_{f} \times 250 = 0.5 \times 50 + 0.25 \times 150$
$M_{f} = 0.25 M$
Hence, option $D$ is correct.

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